Heat & Thermodynamics
The ionization constant of chloroacetic acid is 1.35×10−3. What will be the pH of 0.1 M acid and its 0.1 M sodium salt solution?
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What is the hydrolysis constant of the OCl− ion? The ionization constant of HOCl is 3.0×10−8.
Variation of equilibrium constan K with temperature is given by van't Hoff equation InK=RΔrS∘−RTΔrH∘ for this equation, (ΔrH∘) can be evaluated if equilibrium constans K1 and K2 at two temperature T1 and T2 are known. log(K1K2)=2.303RΔrH∘[T11−T21] For an isomerization X(g)⇔Y(g) the temperature dependency of equilibrium cohnstant is given by : lnK=2−T1000 The value of ΔrS∘ at 300K is :
Given the following Ka values, determine which species is the strongest base ? HSO4−=1.2×10−2,H2PO4−=6.3×10−8,HCO3−=4.7×10−11
Given : Enthalpy of ioinization of two acids : △H∘(HCN)=45.2KJmol− △H∘(CH3COOH)=2.1KJmol− which relationshop for the two acids is true ?
Which of the following solutions has the highest pH?
For a gaseous reaction aA(g)+bB(g)⇔cC(g)+dD(g) equilibrium constants Kc,Kp and Kx are represented by the following reation Kc=[A]a[B]b[C]c[D]d,Kp=PAaPcc.PDd and Kx=xAa.xBbxCc.xDd where [A] represents molar concentrationof A,pA represents partial pressure of A and P represents total pressure, xA represents mole fraction of A On the basis of above work-up select the write option
If degree of dissociation is 0.01 of decimolar solution of weak acid HA then pKa of acid is :
Each question contains STATEMENT-1 (Assertion) and STATEMENT-2( Reason). Examine the statements carefully and mark the correct answer according to the instruction given below: STATEMENT-1: Equilibrium constant for the reverse reaction is the inverse of the equilibrium constant for the reaction in the forward direction. STATEMENT-2: Equilibrium constant depends upon the way in which the reaction is written.